[PDF] arrhenius equation notes

The Arrhenius equation's exponential portion (-Ea/R.T.) reports an increase in the rate constant value with any activation energy decrease. As the chemical reaction rate depends on the reaction's rate constant, the reduction in activation energy yields an exclusive increment in the rate of reaction.
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  • What is the Arrhenius equation and explain the terms?

    Arrhenius equation
    Note: The Arrhenius equation is sometimes expressed as k = Ae-E/RT where k is the rate of chemical reaction, A is a constant depending on the chemicals involved, E is the activation energy, R is the universal gas constant, and T is the temperature.

  • What is the importance of Arrhenius equation?

    The Arrhenius equation is used for calculating the rate of reaction.
    It is a crucial part in chemical kinetics. It helps to understand the impact of temperature on the rate of reaction.
    This equation was first introduced by Svente Arrhenius in 1889.

  • How is activation energy derived from the Arrhenius equation?

    Derivation of Activation Energy
    A = pre-exponent which is a constant.
    Taking log on both sides of the equation.
    It can also be derived mathematically by taking the A1,A2 and T1,T2 values into the arrhenius equation.

  • How is activation energy derived from the Arrhenius equation?

    The basic assumptions of the Arrhenius theory is the collision theory.
    The Arrhenius equation ( k = A e ? E a R T ) establish a relationship between the the rate constant of a reaction ( ) to the frequency factor ( ) and the activation energy of the reaction ( ).

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